[3] Nitrogen dioxide gas (NO2) decomposes slowly to nitrous oxide (NO) and oxygen (O,) at 383 °C. At 383 °C theconcentration verses time data were collected for this reaction, and a plot of 1/[NO2] verses time resulted in astraight line with a slope of 4.7/M-s. If the initial concentration of NO2 = 0.600M.(a) Determine the rate law.(b) Determine the value of the rate constant, k.(c) How long will it take for 40 % the NO, to be converted to product?

Given : We have to calculate rate law and rate constant and time.

Nitrogen dioxide gas (NO:) decomposes slowly to nitrous oxide (NO) and oxygen (O2) at 383 °C. At 383 °C th centration verses time data were collected for this reaction, and a plot of 1/[NO2] verses time resulted in a ight line with a slope of 4.7/M•s. If the initial concentration of NO2 = 0.600M. Determine the rate law. Detemine the value of the rate constant, k. How long will it take for 40 % the NO; to be converted to product?

Nitrogen dioxide gas (NO:) decomposes slowly to nitrous oxide (NO) and oxygen (O2) at 383 °C. At 383 °C th centration verses time data were collected for this reaction, and a plot of 1/[NO2] verses time resulted in a ight line with a slope of 4.7/M•s. If the initial concentration of NO2 = 0.600M. Determine the rate law. Detemine the value of the rate constant, k. How long will it take for 40 % the NO; to be converted to product?

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter13: Chemical Kinetics

Section: Chapter Questions

Problem 13.23QE: Nitrogen monoxide reacts with chlorine to form nitrosyl chloride. NO(g)+12Cl2(g)NOCl(g) The figure...

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